3.2 mole of iodide were heated in a sealed bulb at 444 degree C till the equilibrium was reached. The degree of dissociation of HI at this temperature was found to be 22% . The number of moles of hydrogen iodide present at equilibrium are :

  • Option 1)

    2.496

  • Option 2)

    1.87

  • Option 3)

    2.00

  • Option 4)

    4.00

 

Answers (1)

As we learned in concept

Law of Chemical equilibrium -

At a given temperature, the product of concentration of the reaction products raised to the respective stoichiometric coefficient in the balanced chemical equation divided by the product of concentration of the reactants raised to their individual stoichiometric coefficients has a constant value.

- wherein

aA+bB\rightleftharpoons cC+dD


K_{c}=\frac{[C]^{c\:[D]^{d}}}{[A]^{a}\:[B]^{b}}

[A],\:[B],\:[C]\:[D]

are equilibrium concentration

 

 The reaction undergoes as follows:

                                          2HI\:\rightleftharpoons \:H_{2}+I_{2}

At  t=0                                3.2                0         0

At equilibrium               3.2(1-\propto )   3.2\propto  3.2\propto

\propto\:=\:0.22\:(given)

Number of moles at HI at equilibrium = 3.2 (1-0.22)

                                                              = 3.2 x 0.78 = 496 mol


Option 1)

2.496

This option is correct.

Option 2)

1.87

This option is incorrect.

Option 3)

2.00

This option is incorrect.

Option 4)

4.00

This option is incorrect.

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